CH 18 Solutions Flashcards
Moles of solute dissolved in 1 liter of solution
Molarity
Moles of solute dissolved in 1kg or 1000g of solvent
Molality
Ratio of moles of solute per total moles
Mole Fraction
A solution containing the maximum amount of solute
Saturated
A solution containing less than the maximum amount of solute
Unsaturated
A solution containing more solute than can theoretically dissolve at a given temperature
Supersaturated
Solution containing a large amount of solute
Concentrated
Solution containing a small amount of solute
Diluted
Liquids that are soluble in one another
Miscible
Liquids that are not soluble (insoluble) in one another
Imiscible
At a given temperature solubility of a gas in a liquid is directly proportionate to the pressure of the gas above the liquid
Henry’s Law
Measure of the amount of solute dissolved in specified quantity of solvant
Concentration
Depends on the number of particles a solute yields in a solution
Colligative Property
A colligative property related to the fact that ice will form at higher temperatures in the great lakes than the ocean
Freezing point depression
A colligative property related to the fact that a decrease in the vapor pressure of a solution
Boiling point elevation
If temperature increases, what happens to the solubility of the gas?
It decreases
Solids and liquids ____ solubility with temperature, gas ______
increase, drecreases
What are 3 thing you can do to increase the rate of solution formation?
- Agitation/mixing
- Increasing surface area/breaking it up
- Increasing temperature
Does an increase in pressure affect the solubility of solids or liquids?
No
Does an increase in pressure increase solubility of gas?
Yes
Remember for substances to be miscible they have to:
- Both be liquids
- The same-ish *like dissolves like
Examples:
- Salt dissolves in water
- Tar dissolves in oil
What will not dissolve in water?
Anything Nonpolar
Dilution math equation:
M₁V₁=M₂V₂
Molarity math equation:
Moles of solute/Liter of solution (V)
Moles of solute (In molarity equation)=
g solute/molar mass solute
1L=?ml
1000ml
